The minimum energy a molecule should possess in order to enter into a fruitful collision is known as

The rate constant for a first order reaction is $0.58 \ s^{-1}$ at $300 \ K$ and $0.026 \ s^{-1}$ at $290 \ K$. What is the energy of activation? $(R=8.314 \ J \ K^{-1} \ mol^{-1})$

What do $Z_{AB}$ and $P$ indicate in the context of collision theory?

What is the relationship between the temperature $T$ and the activation energy $E_a$ in the Arrhenius equation?

At $300 \ K$,the activation energy and rate constant for the given reaction are $10 \ kJ \ mol^{-1}$ and $2.4 \times 10^{-5} \ s^{-1}$ respectively. At what temperature (in $K$) will the value of $t_{1/2}$ be $2 \ hr$?
$2N_2O_5 \to 4NO_2 + O_2$

Which statement is incorrect for collision theory?